Nano Catalyst Pumps Up Fuel Cells

Wednesday, November 10, 2010 @ 04:11 PM gHale

Before large fleets of fuel-cell-powered vehicles can hit the road, there needs to be a way to protect platinum, the most expensive component of fuel-cell technology, and to reduce the amount needed to make catalytically active electrodes.
A new electrocatalyst is under development that uses a single layer of platinum and minimizes its wear and tear while maintaining high levels of reactivity during tests that mimic stop-and-go driving.
The research may enhance fuel-cell vehicles and may also be applicable for improving the performance of other metallic catalysts, said researchers at the U.S. Department of Energy’s (DOE) Brookhaven National Laboratory.
The newly designed catalysts consist of a single layer of platinum over a palladium (or palladium-gold alloy) nanoparticle core. Their structural characterization occurred at Brookhaven’s Center for Functional Nanomaterials and the National Synchrotron Light Source.
“Our studies of the structure and activity of this catalyst — and comparisons with platinum-carbon catalysts currently in use — illustrate that the palladium core ‘protects’ the fine layer of platinum surrounding the particles, enabling it to maintain reactivity for a much longer period of time,” said Brookhaven Lab chemist Radoslav Adzic, who leads the research team.
In conventional fuel-cell catalysts, the oxidation and reduction cycling — triggered by changes in voltage occurring during stop-and-go driving — damages the platinum. Over time, the platinum dissolves, causing irreversible damage to the fuel cell.
In the new catalyst, palladium from the core is more reactive than platinum in these oxidation and reduction reactions. Stability tests simulating fuel cell voltage cycling revealed that, after 100,000 potential cycles, a significant amount of palladium oxidized, dissolved, and migrated away from the cathode. In the membrane between the cathode and anode, the dissolved palladium ions ended up reduced by hydrogen diffusing from the anode to form a “band,” or dots.
In contrast, platinum was almost unaffected, except for a small contraction of the platinum monolayer. “This contraction of the platinum lattice makes the catalyst more active and the stability of the particles increases,” Adzic said.
Reactivity of the platinum monolayer/palladium core catalyst also remained extremely high. It reduced by 37 percent after 100,000 cycles.
Building on earlier work that illustrated how small amounts of gold can enhance catalytic activity, the scientists also developed a form of the platinum monolayer catalyst with a palladium-gold alloy core. The addition of gold further increased the stability of the electrocatalyst, which retained nearly 70 percent of reactivity after 200,000 cycles of testing.
“This indicates the excellent durability of this electrocatalyst, especially when compared with simpler platinum-carbon catalysts, which lose nearly 70 percent of their reactivity after much shorter cycling times. This level of activity and stability indicates that this is a practical catalyst. It exceeds the goal set by DOE for 2010-2015 and it can be used for automotive applications,” Adzic said.
He noted that fuel cells made using the new catalyst would require only about 10 grams of platinum per car — and less than 20 grams of palladium. Currently, in catalytic convertors used to treat exhaust gases, they use 5 to 10 grams of platinum. Since fuel-cell-powered cars would emit no exhaust gases, there would be no need for such catalytic converters, and therefore no net increase in the amount of platinum used.
“In addition to developing electrocatalysts for automotive fuel cell applications, these findings indicate the broad applicability of platinum monolayer catalysts and the possibility of extending this concept to catalysts based on other noble metals,” Adzic said.

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